2. Match a formula in the right column with its appropriate name in the left column.

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1 UNIT 3: CHEMICAL BONDING. CHEMICAL COMPOUNDS Content: Unit 3 Chemical bonding. Chemical compounds 3.1. Chemical bonding 3.2. Chemical compounds Oxides Hydroxides Hydrides Binary acids Oxy-acids Salts 3.3. Nomenclature and Formulas Learning Aims: At the end of the unit, the student will know: Atoms bond together with other atoms to make a compound. To formulate and name different chemical compounds: oxides, hydroxides, hydrides, hydracids, oxy-acids and Salts To use the appropriate language to answer questions and to communicate with teacher and classmates. Initial Activities 1. Choose the right statement: a) Oxides are made of oxygen and another element. b) A covalent bond occurs between a metal and a non-metal element. c) Ionic bond involves electron sharing. d) When an atom loses an electron it becomes negatively charged. 2. Match a formula in the right column with its appropriate name in the left column. Ammonia CO 2 Sodium hydroxide H 2 SO 4 Sulphuric acid NH 3 Carbon dioxide KCl Hydrochloride acid HNO 3 Potassium Chloride NaOH Nitric acid HCl 32

2 Key words: Ionic bond Na + Cl - Electrical forces Chemical bond between metal and non-metal ions through electrostatic forces (video, simulation of ionic bond) =55 (reaction of sodium and chlorine) Forces that bond atoms or molecules together are of electrical character Covalent bond Chemical bond characterized by the sharing of pairs of electrons between atoms. (video, single covalent bond) Hydrogen bond Attractive force between the hydrogen attached to an electronegative atom (N, O or F) of one molecule and an electronegative atom (N, O or F) of a different molecule. Van der Waals bond Intermolecular attraction between one molecule and a neighbouring molecule. Metallic bond Chemical bond in which mobile valence electrons (electron gas) are shared among positive metallic ions in a crystalline structure Negative ions Cl - Atom or molecule that gains electrons and becomes electrically charged. 33

3 Positive ions Na + Atom or molecule that loses electrons and becomes electrically charged. Oxides Binary compound of an element with oxygen. (dictionary with pronunciation) Hydroxides Chemical compound containing hydroxyl radicals (OH - ). Hydrides Compounds of hydrogen with a metal. Hydracids Acids that does not contain oxygen. Oxy-acids Acids that contain hydrogen, oxygen and a non-metal element. Salts Chemical compound formed by replacing all or part of the hydrogen ions of an acid with metal ions or electropositive radicals. (Dictionary with pronunciation) 34

4 3.1. Chemical bonding Atoms bond with another atom to make molecules or molecular aggregates. Atoms are held together by chemical bonds, attractive forces that keep together the atoms. A bond is formed when valence electrons (atoms that occupies the outermost electron cell) from two atoms interact with each other. We can differentiate five types of bonds: 1. Covalent bond: two atoms share valence electrons between them. Covalent bonds are between non-metals and non-metals or hydrogen and non-metals. They share electrons so that both of them can have a stable octet. (simulation of covalent bond) 2. Ionic bond: one atom gains a valence electron (forming a negative ion called anion) from a different atom, this atom loses the electron and a positive ion or cation is obtained. These oppositely charged ions are attracted to each other, forming an ionic bond. The ionic bonds are between metals and non-metals. (simulation of ionic bond) 3. Metallic bonding: atoms lose valence electrons; these mobile valence electrons (electron gas) are shared among positive metallic ions in a crystalline structure. This is the characteristic bonding of metals. 35

5 4. Van der Waals bond: intermolecular attraction between one molecule and a neighbouring molecule. 5. Hydrogen bond: attractive force between the hydrogen attached to an electronegative atom (N, O or F) of one molecule and an electronegative atom (N, O or F) of a different molecule. More information: Questions 1. Choose the correct answer: 1.1. Non-metals and non-metals tend to form. bond. a) Covalent. b) Ionic c) Metallic 1.2. Metals and non-metals tend to form. bond. a) Covalent. b) Ionic c) Metallic 1.3. Non-metals and hydrogen tend to form. bond. a) Covalent. b) Ionic c) Metallic 1.4. Non-metals tend to electrons to become ions. a) gain, negative. b) lose, positive. c) gain, positive d) lose, negative 36

6 1.5. Metals tend to electrons to become ions. a) gain, negative. b) lose, positive. c) gain, positive d) lose, negative 1.6. When an atom of magnesium loses two electrons, it gets a charge a) +2. b) When an atom of sulphur gains two electrons, it gets a charge a) +2. b) Negative ions are called a) electrons. b) protons. c) anions. d) cations Positive ions are called a) electrons. b) protons. c) anions. d) cations. 2. Match one formula of left column with their corresponding bond in right column. O 2 NaCl HCl H 2 O Al n SO 2 CaS Covalent Ionic Metallic 3. Write down the ions formed by the following elements: a) Sodium b) Beryllium c) Fluorine d) Sulphur e) Aluminium 37

7 3.2. Chemical compounds A chemical compound is a substance formed by chemical union of two or more different elements bounded together in definite proportion by mass. The elements of a compound can not be obtained from the compound by physical methods. Later we will speak about different inorganic compounds: Oxides Oxides are binary compound of an element with oxygen. Example: Fe 2 O 3 : Iron (II) oxide Hydroxides Hydroxides are chemical compounds containing hydroxyl radicals (OH - ). Example: NaOH: Sodium hydroxide Hydrides These chemicals compounds are a combination of hydrogen with another element. Example: NaH: Sodium hydride Binary acids These acids do not contain oxygen; they contain hydrogen and a no-metal element of group 16 or 17 of the Periodic Table. Example: HCl: Hydrochloric acid Oxy-acids Oxy-acids contain hydrogen, oxygen and usually a non-metal element. Example: HClO 4 : Perchloric acid Salts Salts are formed by replacing all or part of the hydrogen ions of an acid with metal ions or electropositive radicals. Example: Na 2 SO 4 : Sodium sulphate 38

8 3.3. Nomenclature and Formulas Now is the time to learn a few rules of the IUPAC nomenclature of inorganic chemistry (International Union of Pure and Applied Chemistry) to name and formulate inorganic compounds): 1. In binary compounds a) The more electropositive element is placed first in the formula. b) The more electronegative element is written last and with an -ide suffix 2. Before each element prefixes are used to indicated the number of atoms: 1 (mono-); 2 (di-); 3 (tri-); 4 (tetra-); 5 (penta-); 6 (hexa-); 7 (hepta-); 8 (octa-); 9 (nona-); 10 (deca-). Exception: The prefix mono- is not used with the first element. Example: NO: nitrogen monoxide; 3. Ion OH - is called hydroxide. Example: KOH: potassium hydroxide 4. Ion H - is called hydride Example: NaH: sodium hydride 5. There are some binary compounds with common names: BH 3 : Borane; NH 3 : Ammonia; PH 3 : Phosphane; CH 4 : Methane 6. Binary acids follow the pattern of hydroelementic acid Example: HBr: hydrobromic acid 7. Ternary acids follow the pattern of hipoelementous, elementous, elementic, perelementic, acid, depending on the valence of central atom. Example: HBrO 3 : bromic acid 8. Some elements form two or more different ions with different charges. To distinguish the compounds, its charge is included with its name as a Roman numeral in parentheses. Example: Fe 2 O 3 : iron (III) oxide; FeO: iron (II) oxide 9. In oxy-salts suffix ous of acid is changed by ite and the suffix ic by ate Example: NaNO 3 : sodium nitrate Oxy-anions names CO 3 2- Carbonate ion NO 2 - : Nitrite ion NO 3 - : Nitrate ion PO 3 3- : Phosphite ion PO 4 3- : Phosphate ion SO 2 2- : Hyposulphite ion SO 3 2- : Sulphite ion SO 4 2- : Sulphate ion ClO - : Hypochlorite ion ClO 2 - : Chlorite ion ClO 3 - : Chlorate ion ClO 4 - : Perchlorate ion 39

9 Questions 1. Choose the correct answer: 1.1. The chemical formula of the product formed from the reaction between hydrogen and chlorine is: a) HCl b) H 3 Cl c) H 5 Cl 1.2. The chemical formula of calcium oxide is: a) Ca 2 O b) CaO c) CaO The chemical formula of potassium chloride is: a) K 2 Cl b) KCl 2 d) KCl 1.4. The chemical formula of potassium sulphate is: a) K 2 SO 3 b) KS 2 e) KSO 4 f) K 2 SO 4 2. Write the chemical formula for a compound that has a) one calcium atom and 1 sulphur atom. b) two iron atoms and three oxygen atoms. c) one aluminium atoms and three hydroxyl groups d) one nitrogen atom and three hydrogen atoms. 3. Write the formula for: dinitrogen monoxide nitrogen monoxide dinitrogen trioxide dinitrogen pentoxide carbon monoxide carbon dioxide sodium chloride zinc iodide 40

10 4. Match the formulas on the left to their names on the right. NaOH HNO 3 Al(OH) 3 HF Ca(OH) 2 H 3 PO 4 HClO 2 HClO 3 HCl NaNO 3 H 2 CO 3 KClO H 2 SO 3 KOH NH 4 OH CaSO 4 Fe(OH) 3 HBr H 2 CrO 4 H 2 S Mg(OH) 2 H 2 SO 4 hydrochloric acid sulphuric acid carbonic acid potassium hydroxide aluminium hydroxide sulphurous acid sodium nitrate nitric acid hydrobromic acid ammonium hydroxide calcium sulphate phosphoric acid chromic acid potassium hypochlorite magnesium hydroxide hydrosulfuric acid hydrofluoric acid calcium hydroxide chlorous acidunit sodium hydroxide chloric acid iron(iii) hydroxide 5. Give the name for the following formulas: NaNO 3 Ag 2 CO 3 (NH 4 ) 2 SO 4 CuO Cu 2 O Cr 2 O 3 HCl HBr H 2 S HClO 3 H 2 SO 4 HNO 3 H 3 PO 3 HClO 2 HClO 41

11 6. Word search: look for ten words related to nomenclature 7. Criss-cross Across 1. Chemical bond between two ions with opposite charges 3. Compound of hydrogen with another element. 4. Common name of calcium carbonate 6. Chemical bond formed by the sharing of one or more electrons between atoms 7. Name of an element and of a type of bond 8. Substance having a sour taste Down 2. Binary compound of an element or radical with oxygen 4. Chemical bond characteristic of metals 5. Common name of sodium hypochlorite 42

12 STUDENT SELF-EVALUATION CHECKLIST (WHAT STUDENTS HAVE LEARNT) 1.- When you know the meaning of the following words, tick the box: Covalent bond Ionic bond Metallic bond Hydrogen bond Van der Waals bond Oxide Hydroxide Hydride Acid Salt 2.- Tick the one you think is your answer: I know that in covalent bond electrons are sharing. I know that an ionic bond occurs by the attraction of positively charged metal and a negatively charged non metall. I know that in metallic bond a cloud of electrons is moving around a crystalline structure of positive ions of metallic elements. I understand the meaning of a chemical formula. I know how to formulate oxides, hydroxides, hydrides and the most common inorganic acids and salts. I know very well I need some revision I need some more help 3.- What ideas or parts of this unit do you think are: - More interesting. - Not enough explained. - More difficult. - Best learned. - Boring - Not enough worked. 4.- Tell the tasks you have done the best. 5.- Tell the tasks you have done incorrectly. 6.- If you have some problem to name or formulate chemical compound, specify it. 43

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